C2: BONDING

Question 1

Ionic bonding

Answer 1

-electrons transferred from metal to non-metal
-strong electrostatic forces of electrons between oppositely charged ions
-giant ionic structure

Question 2

Properties of ionic compounds

Answer 2

-high melting and boiling points (strong electrostatic forces require lots of energy to overcome)
-can’t conduct electricity as a solid (can’t carry a charge through the structure as electrons are not free to move)
-conduct electricity as a liquid (can carry a charge through the structure as electrons are free to move)

Question 3

Simple molecular bonding

Answer 3

-electrons shared between non-metals
-weak intermolecular forces
-simple molecular structure

Question 4

Properties of simple molecular bonds

Answer 4

-low melting and boiling points (weak intermolecular forces require little energy to overcome)
-don’t conduct electricity as a solid or a liquid (no delocalised electrons to carry a charge through the structure)

Question 5

Metallic bonding

Answer 5

-bonding between metals
-strong electrostatic forces of attraction between +ve ions and delocalised electrons
-giant structure

Question 6

Properties of metals

Answer 6

-high melting and boiling points (strong electrostatic forces require lots of energy to overcome)
-conduct electricity (delocalised electrons can carry a charge through the structure)
-malleable (layers can slide over each other)

Question 7

Why are alloys harder than pure metals?

Answer 7

alloys have different sized atoms which distorts the layers meaning that they can’t slide over each other

Question 8

Why do alloys not conduct electricity?

Answer 8

alloys have different sized atoms which distorts the layers meaning that delocalised electrons can’t carry a charge through the structure

Question 9

Giant covalent bonding

Answer 9

-bonding between non-metals
-strong covalent bonds
-giant covalent structure

Question 10

Properties of diamond

Answer 10

-strong (each carbon atom is bonded to 4 others with strong covalent bonds)
-high melting and boiling points (strong covalent bonds require lots of energy to break)
-doesn’t conduct electricity (no free electrons or ions)

Question 11

Properties of graphite

Answer 11

-soft and slippery (weak intermolecular forces between layers)
-conducts electricity (each carbon atom only bonds to 3 others so each carbon atom has a delocalised electron that can carry a chsrge through the structure
-high melting and boiling points (strong covalent bonds require lots of energy to break)